Assuming that $Ba(OH)_{2}$ is completely ionised in aqueous solution under the given conditions,the concentration of $H_{3}O^{+}$ ions in $0.005 \, M$ aqueous solution of $Ba(OH)_{2}$ at $298 \, K$ is $..... \times 10^{-12} \, mol \, L^{-1}$. (Nearest integer)
- A$2$
- B$1$
- C$3$
- D$4$
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Similar Questions
Select the correct option that has the same $pH$ value.
$(1) 0.005 \, M \, H_2SO_4$
$(2) 0.1 \, M \, Na_2SO_4$
$(3) 10^{-2} \, M \, NaOH$
$(4) 0.01 \, M \, HCl$
$(1) 0.005 \, M \, H_2SO_4$
$(2) 0.1 \, M \, Na_2SO_4$
$(3) 10^{-2} \, M \, NaOH$
$(4) 0.01 \, M \, HCl$
Medium
View Solution$50 \ mL$ of $H_2O$ is added to $50 \ mL$ of $1 \times 10^{-3} \ M$ barium hydroxide solution. What is the $pH$ of the resulting solution?
DifficultTS EAMCET 2008
View SolutionCalculate the $pH$ of a $0.002 \ M$ $KOH$ solution.
If $1 \ mL$ of $1 \ M \ HCl$ solution is added to $99 \ mL$ of aqueous solution of $NaCl$,the $pH$ of the solution changes by $X$ units. The value of $X$ is:
Medium
View SolutionFor a solution of $HCl$ assuming complete ionization,the $pH = 1$. Find the normality of a $H_2SO_4$ solution having the same $pH$.
Medium
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